Q: Consider the following data. For the acid: HA- Ka = 7.46⋅10−87.46⋅10-8 Calculate the Kb for A2-.…
A: Kb is the base dissociation constant. The base dissociation constant is a measure of how completely…
Q: Calculation of pH (SHOW CALCULATION FROM THE GRAPH IATTACH GRAPHI 2.Find out pH at equivalent to…
A: Plot of pH vs Volume of NaOH added
Q: The Ka for an acid is 7.91 x 10-29. Calculate the pKa for this acid.
A: The pKa for the acid is to be calculated
Q: A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A¯(aq)…
A: Given, the dissociation equation for the weak acid, HA: HA (aq) ⇌ H+ (aq) + A- (aq) Given the…
Q: What is the pKa of an acid? As the pKa value increases, does the acid strength increase or…
A: The pKa value is method used for indicate the strength of an acid. pKa is the negative log of the…
Q: Write the expression for Ka of H2PO4- in terms of concentration of relevant species. H2PO4- + H2O…
A: The dissociation reaction of H2PO4- ion is H2PO4- (aq) + H2O (l) -------> HPO42- (aq) + H3O+ (aq)…
Q: Write the expresson for the dissociation constant, Ka for an aqueous solution of butanoic acid.…
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Q: Use pka values to predict which of the following equilibria will favor the reactants.
A:
Q: Determine what is wrong with the Ksp expression for Ba(OH)2 and correct it. [Ba(OH)2] Ksp [Ba*][OH…
A: as per Q&A guidelines of portal I solve first question because it comes under multiple question…
Q: What is the electrostatic force of repulsion for two protons separated by 75 pm.
A: The electrostatic force of repulsion for two protons is calculated as,
Q: For the second dissociation of H, CO3: HCO3(aq) + H,O=H;O) + COaq) + CO3(aq) (1) a. At what volume…
A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
Q: The Ka of a weak acid is 3 x 10^-12 What is the pKa of this acid?
A: Ka which is dissociation constant of acid is given 3*10^-12 Pka = ?
Q: Calculate the acid ionization constant (pKa) for the acid with a 0.775 M solution of a weak acid…
A: Given data of the following:: [weak acid] = 0.775 M = [HA] pH = 3.38 pka = ?
Q: 60°C, water has an autoionization constant (Kw) of 9.247 X 10-14. Determine the pOH of pure water at…
A: Given- Kw=9.247×10^-14 Temperature=60°C pOH=?
Q: Write the MBE, PBE and CBE for the following: a. 0.15M H2CrO4 b 0 35M KCIO,
A: Charge Balance Equation (CBE): It is based on electroneutrality principle. The molar concentration…
Q: propiophenone + excess Br2 + excess NaOH=
A: Given: Propiophenone + excess Br2 + excess NaOH
Q: Ka for hydrofluoric acid is 6.8 x 104. What is the first digit of the pK value for hydrofluoric…
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Q: The dissociation constant, ka, of a weak acid is 5.9 x 10-6. What is the pKa of the acid?
A:
Q: Calculate the Ksp of the following compounds, given their molar solubilities. (a) Cus, 7.33 x 10-19…
A: Calculate Ksp by using molar solubility ---
Q: When solid ammonium hydrogen sulfide, NH4SH, undergoes thermal decomposition, ammonia gas, and…
A:
Q: What is the accepted value for the Ksp of Ca(OH)2, including the conditions for its determination
A: Given What is the accepted value for the Ksp of Ca(OH)2, including the conditions for its…
Q: What is the ratio of conjugate base to undissociated acid for a weak acid with a pk, of 4.4 at a pH…
A: Given : pKa = 4.4 pH = 9 To determine : Ratio of conjugate base to weak acid
Q: [b] Derive the following question ;- pH = pK, + log [ Cs/C.1
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Q: A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A (aq)…
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Q: The pKa for the first protonation of nicotine (2) is 8.02. What is the pH and the fraction of…
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Q: The acid dissociation constant K, of trimethylacetic acid (HC(CH;),CO2) is Calculate the pH of a 1.4…
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Q: 1. If the Ka of an acid is 1.8x10 ^-5, calculate the pKa and pKb values of the acid.
A: Since you have asked multiple type questions, we will solve only first questions for you. If you…
Q: What is the effect of pH on protein solubility? What is the isoelectric point (pI) of soy protein?
A: Proteins :- A protein is a naturally occurring organic compound, extremely complex substance…
Q: Which solution is closest to the pKa? Calculate the pH of the solutions and the change in pH after…
A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…
Q: What is the pH of a 0.20 M solution of sodium acetate? The Ka for acetic acid is 1.8 x 10⁻⁵?
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Q: Determine the pka of an acid whose concentration is 0.100M and pH is 2.86.
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Q: 3. Consider the following acids Acid Acetic Acid, H CCO-H Trichloroacetic Acid, Cl-CCO,H…
A:
Q: pkal pK₂2 Phosphoric acid, H, PO, (aq), is a triprotic acid, meaning that one molecule of the acid…
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Q: Summarize the application of qualitative chemistry in refining crude oil
A: Given Summarize the application of qualitative chemistry in refining crude oil
Q: Consider two acids: CH;CO,H (benzoic acid, pK, = 4.2) and CH,CO,H (acetic acid, pK,= 4.8). Which…
A: According to Bronsted-Lowry concept Acid is a substance which donates proton to other and forms its…
Q: Which of the following is not used to be standardized against KHP? a. H2SO4 b. NaOH c. NH3 d.…
A: The following is not used to be standardized against KHP is given below.
Q: Consider the following data: HX ↔ X− + H+HX ↔ X- + H+ Ka =…
A: Given reactions HX ↔ X− + H+ Ka = 6.83×10-6 H2A ↔ HA− + H+ Ka = 6.85×10-8…
Q: provide an explanation of the graphs (a) and (b) the relationship of the biological activity of the…
A: Sulfonamide (also known as sulfa drugs) is the fundamental functional group of more than a few…
Q: Calculate the Ka of HA given A−(aq)+H2O(l)⇌OH−(aq)+HA(aq) Kb = 9.60×10-7
A: Given reaction : A-(aq.) + H2O(l) ⇌ OH-(aq.) + HA(aq.) Kb = 9.60×10-7 We can use the relation…
Q: Given a solution of 0.0025 M HC2H3O2, Ka = 1.8 x 10^-5 a. Calculate the pH of the solution. b.…
A: The question is based on the concept of equilibrium. we have to calculate the pH of the acetic acid…
Q: The amino acid tyrosine has pKa = 2.20 for deprotonation of its carboxylic acid group. What are the…
A: Henderson-Hasselbalch equation establishes a relationship between pH of the solution and the acid…
Q: Write the reaction as proton-transfer reactions. Label which reactant is the acid and which is the…
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Q: The pH of a saturated solution of metal hydroxide, Me(OH)2, is 12.4 at room temperature. Calculate…
A:
Q: The dissociation constant (Ka) of a weak acid is 1.8 x 10, calculate the pKa of the this weak acid.…
A: Ka of weak acid = 1.8 × 10-5 pKa of weak acid = ?
Q: KOAC PPy
A: Given is a palladium catalysed reaction. This is an example of intermolecular Heck reaction of Aryl…
Q: The pKa of HX is 9.34. Calculate the pH of a 0.418 M solution of HX.
A: We are authorized to answer one question at a time, since you have not mentioned which question you…
Q: (b)Given the K, and pK values of the following compounds: Hydrobromic acid (HBr), K= 1.0 x 10;…
A: Solution: We have general knowledge about pH , pKa. From the pKa we can know about the acidic…
Define pKa and provide at least one method for determining its value.
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- What is the accepted value for the Ksp of Ca(OH)2, including the conditions for its determination?Write the balanced chemical equation for conversion of Al(s) to KAl(SO4)2·12H2O(s) in aqueous solution. Equation 1 - 2Al(s) + 2K+(aq) + 2OH-(aq) + 10H2O(l) --> 2K+(aq) + 2[Al(H2O)2(OH)4)-(aq) + 3H2(g) Equation 2 - 2K+ (aq) + 2[Al(H2O)2(OH)4]-(aq) + 2H+(aq) + SO42-(aq) --> 2K+(aq) + SO42-(aq) + 2Al(H2O)3(OH)3(s) Equation 3 - 2Al(H2O)3(OH)3(s) + 6H+(aq) + 3SO42-(aq) --> 2Al3+(aq) + 3SO42-(aq) + 12H2O(l) Equation 4 - K+(aq) + Al3+(aq) + 2SO42-(aq) --> KAl(SO4)2∙12H2O(s)Carbonic acid, H2CO3, undergoes the following acid base equilibria: H2CO3,=H*(aq) + HCO3 (aq) =H*(aq) + CO3² (aq). The pKa values for the first and second steps are 3.6 and 6.3, respectively. The pH of human blood is 7.37 and this is tightly regulated. Which of the following statements most accurately describes the concentrations of the different species in the above reaction. A) [H2CO3(aq)] is much larger than the other species B) [H¿CO3(aq)] and [HCO3¯(aq)] are much larger than the other species C) [HCO3 (aq)] and [CO32 (aq)] are much larger than the other species D) [CO3? (aq)] is much larger than the other species
- 3) One of the main buffer systems found in living organisms is the phosphate buffer system, often used in biological research to mimic cellular conditions. The phosphate equilibrium reactions and their corresponding pKa's are as follows: H3PO4 = H* + H2PO, H2PO, = H+ + HPO?- HPO- = H+ + PO;- pKa1 pКаz —D 7.21 = 12.44 = 2.12 pKa3 (a) Given the above chemical reaction, write out the expression for K, of the buffer system which would predominate at neutral pH conditions. Justify your choice. (b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to maintain homeostasis. However, some more acid-tolerant or basic-tolerant organisms can survive (and sometimes thrive) within different ranges of pH. Calculate the mass and moles of the correct acid and corresponding conjugate base solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO4, and Na PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total, including the concentration of acid and base…Explain the chemistry behind ocean acidification. You should include the formation of carbonic acid from carbon dioxide, how this reacts with carbonate ions, and how continued CO2 emission will impact ocean pH.Coral structures found in the Great Barrier Reef are composed of calcium carbonate, CaCO3, and are under threat of dissolution due to ocean acidification. Consider the following equilibrium reaction equation. CaCO3(s) + CO2(aq) + H2O(l) ⇌ Ca2+(aq) + 2HCO3–(aq) Write the expression for the equilibrium constant, Kc for this reaction. Predict whether the pH of the ocean will increase or decrease as a result of a decrease in the partial pressure of carbon dioxide in the atmosphere (circle your answer). Calculate the molar solubility (s) of calcium carbonate in water at 25 °C when Ksp = 4.5 ´ 10–9.
- The value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (a) Write the chemical equation for the equilibrium that corresponds to Ka.Lakes have a natural buffering capacity, especially in regions where limestone gives rise to dissolved calcium carbonate. Write an equation for the effect of a small amount of acid rain containing sulfuric acid if it falls into alake containing carbonate (CO3-2 ) ions. Discuss how the lake will resist further pH changes. What happens if a large excess of acid rain is deposited?Use the systematic treatment of equilibrium to calculate the concentration of Ba2+ in acidic solution, if its concentration is governed by the following equilibria – BaSO4 (s) → Ba2+ + So Ksp = 1.1 x 10-10 so, +H2O HSO, +OH K, = 9.8 x 10-13 Bat + So, BaSO4 (aq) K = 1.9 x 10 Hint: Since the pH is fixed at 1.89, the charge balance is invalidated. Use the mass balance for your calculation.
- Most reaction do not go to completions. Equilibrium is established between the reactants and products. For the reaction of A with B to produce C and D, we can write the chemical equation as: аА + bв + сс + dD where + represents equilibrium between the reactants and products. The extent to which the reaction proceeds to product formation, at a given temperature, is given by the equilibrium constant, Kę. The equilibrium constant is written mathematically (for the above equation) as: [C[[D]* K. = [A]°[B]" where, a, b, c, and d are the stoichiometric coefficients from the balanced chemical equation and the brackets, [ ], indicate molar concentration. 1. For the following reaction: 2A + В + 3с calculate the equilibrium constant, K, if at equilibrium the concentration of A is 0.15M, the concentration of B is 0.20M, and the concentration of C is 0.10M.Calculate the value of the equilibrium constant, Kc, for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Kc = M(g) = Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9 R(g) Kel : 3.49 Kc2 = 0.469 Kc3 = 14.4An aqueous solution of CH3COOH is found to have the following equilibrium concentrations at 25°C: CH3COOH = 1.65a102 M Ht= 5.44x10-4 M CH COO = 5.44x10 4 M Calculate the equilibrium constant, Kc, for the ionization of acetic acid at 25°C. The reaction is CH3COOH(aq) = H(aq) + CH;COO (aq) Type the numerical value only in two significant figures.